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Page 1: Supplemental Problems - d3jc3ahdjad7x7.cloudfront.net · Chapter 24 The Chemistry of Life ... Supplemental Problems Chemistry: Matter and Change • Chapter 2 1 ... c. 26.0 cm 2.1

SupplementalProblems

Page 2: Supplemental Problems - d3jc3ahdjad7x7.cloudfront.net · Chapter 24 The Chemistry of Life ... Supplemental Problems Chemistry: Matter and Change • Chapter 2 1 ... c. 26.0 cm 2.1
Page 3: Supplemental Problems - d3jc3ahdjad7x7.cloudfront.net · Chapter 24 The Chemistry of Life ... Supplemental Problems Chemistry: Matter and Change • Chapter 2 1 ... c. 26.0 cm 2.1

Hands-On Learning:Laboratory Manual, SE/TEForensics Laboratory Manual, SE/TECBL Laboratory Manual, SE/TESmall-Scale Laboratory Manual, SE/TEChemLab and MiniLab Worksheets

Review/Reinforcement:Study Guide for Content Mastery, SE/TESolving Problems: A Chemistry HandbookReviewing ChemistryGuided Reading Audio Program

Applications and Enrichment:Challenge ProblemsSupplemental Problems

Assessment:Chapter AssessmentMindJogger Videoquizzes (VHS/DVD)Computer Test Bank, Windows/MacIntosh

Teacher Resources:Lesson Plans Block Scheduling Lesson PlansSpanish ResourcesSection Focus Transparencies and MastersMath Skills Transparencies and MastersTeaching Transparencies and MastersSolutions Manual

Technology:Chemistry Interactive CD-ROMVocabulary PuzzleMaker Software,

Windows/MacIntoshGlencoe Science Web site: science.glencoe.com

Copyright © 2002 by The McGraw-Hill Companies, Inc.All rights reserved. Permission is granted to reproduce the material contained hereinon the condition that such material be reproduced only for classroom use; be providedto students, teachers, and families without charge; and be used solely in conjunctionwith the Chemistry: Matter and Change program. Any other reproduction, for use orsale, is prohibited without prior written permission of the publisher.

Send all inquiries to:Glencoe/McGraw-Hill8787 Orion PlaceColumbus, OH 43240-4027

ISBN 0-07-824535-4Printed in the United States of America.1 2 3 4 5 6 7 8 9 10 045 09 08 07 06 05 04 03 02 01

A Glencoe Program

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Supplemental Problems Chemistry: Matter and Change iii

To the Teacher . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . iv

Chapter 2 Data Analysis . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 1

Chapter 3 Matter—Properties and Changes . . . . . . . . . . . . . . . . . . . . . 3

Chapter 4 The Structure of the Atom . . . . . . . . . . . . . . . . . . . . . . . . . 5

Chapter 5 Electrons in Atoms . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 7

Chapter 6 The Periodic Table and Periodic Law . . . . . . . . . . . . . . . . . 9

Chapter 10 Chemical Reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 11

Chapter 11 The Mole . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 13

Chapter 12 Stoichiometry . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 15

Chapter 13 States of Matter . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 17

Chapter 14 Gases . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 19

Chapter 15 Solutions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 21

Chapter 16 Energy and Chemical Change . . . . . . . . . . . . . . . . . . . . . . 23

Chapter 17 Reaction Rates . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 25

Chapter 18 Chemical Equilibrium . . . . . . . . . . . . . . . . . . . . . . . . . . . . 27

Chapter 19 Acids and Bases . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 29

Chapter 20 Redox Reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 31

Chapter 21 Electrochemistry . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 33

Chapter 22 Hydrocarbons . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 35

Chapter 24 The Chemistry of Life . . . . . . . . . . . . . . . . . . . . . . . . . . . 37

Chapter 25 Nuclear Chemistry . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 39

Answer Key . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 42

SUPPLEMENTAL PROBLEMS

Contents

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Supplemental Problems Chemistry: Matter and Change • Chapter 2 1

Data AnalysisData Analysis1. A sample of aluminum is placed in a 25-mL

graduated cylinder containing 10.0 mL ofwater. The level of water rises to 18.0 mL.Aluminum has a density of 2.7 g/mL. Calculatethe mass of the sample.

2. Saturn is about 1 429 000 km from the Sun.How many meters is Saturn from the Sun?Write your answer in scientific notation.

3. Use the graph to answer the questions.

a. What kind of graph is this?

b. What are the variables?

c. According to the graph, which has a largerradius, Neptune or Uranus?

d. According to the graph, what is the radiusof Saturn?

e. Convert the radius of Saturn to meters.Write your answer in scientific notation.

4. Look at the graph below. Then answer thequestions.

a. What kind of graph is this?

b. According to the graph, which element ismost abundant in Earth’s crust?

c. According to the graph, what percent ofEarth’s crust is made up of titanium? Ofcalcium?

5. You place a 28.95-g piece of gold in a 10-mLgraduated cylinder. The level of the water rises1.50 mL. What is the density of gold? Youknow that silver has a density of 10.5 g/cm3.What mass of silver will raise the level of thewater in the graduated cylinder 1.50 mL?

6. Convert 55 miles per hour to kilometers perhour. How many kilometers/second is 55 milesper hour? (1 mile � 1.6 km)

7. Convert the following data to scientific notation.

a. 166 000 000 000 000 m2

b. 8847 m

c. 484 liters

The Composition of Earth’s Crust

Oxygen46%

Silicon28%

Aluminum8%

Iron6%

Calcium4%

Magnesium2%

Sodium2%

Potassium2%

Otherelements

1%

Titanium1%

0

5000

15 000

25 000

35 000

45 000

55 000

65 000

75 000

Mer

cury

Ven

us

Eart

h

Mar

s

Jup

iter

Satu

rn

Ura

nu

s

Nep

tun

e

Plu

to

Planet

Rad

ius

(in

km

)

Radii of Planets

SUPPLEMENTAL PROBLEMSCHAPTER 2

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2 Chemistry: Matter and Change • Chapter 2 Supplemental Problems

8. Convert the following as indicated.

a. Aluminum boils at 2467°C. What isaluminum’s boiling point in kelvins?

b. Bromine melts at �7.2°C. What isbromine’s melting point in kelvins?

c. Chlorine melts at 172 K. What is chlorine’smelting point in °C?

d. What is 273 K in °C?

9. American cars use about 600 000 000 gallonsof oil per year. How many liters of oil doAmerican cars use per year? Report youranswer in scientific notation. (1 L � 0.908 quart; 1 gallon � 4 quarts)

Solve the following problems. Express youranswers in proper scientific notation.

10. a. 5.3 � 1012 � 3.0 � 1011 �

b. 3.7 � 106 � 8.0 � 105 �

c. 1.85 � 1016 � 9.25 � 1016 �

d. 2.8 � 1022 � 82 � 1021 �

e. 3.09 � 1020 � 9.1 � 1019 �

f. 17 � 103 � 3 � 104 � 1.3 � 104 �

g. 4.80 � 1015 � 13 � 1013 �

11. a. (4.0 � 105) � (3.0 � 103) �

b. (5.0 � 1012) � (8.05 � 103) �

c. (8.9 � 105) � (3.0 � 103) �

d. (1.6 � 1012) � (8.01 � 10�3) �

e. (9.0 � 105) � (3.0 � 10�3) �

f. (2.4 � 103) � (8.0 � 10�3) �

g. (6.1 � 10�5) � (3.01 � 10�2) �

12. Mac measured the density of silver three timesand obtained the following results:

Trial 1: 10.6 g/cm3; Trial 2: 10.8 g/cm3; Trial 3: 9.6 g/cm3.

Silver has a density of 10.5 g/cm3

a. Calculate Mac’s percent error for each trial.

b. Which trial had the greatest percent error?

13. You calculate that your semester average in history is 97.5. When you get your report card,your average is 96. What was the percent errorof your calculation?

14. Determine the number of significant figures ineach measurement.

a. 0.000 301 5 m

b. 0.121 012 L

c. 1.056 mL

d. 12.90 s

e. 5000 dogs

f. 5.78910 � 103 g

15. Round the number 31.257 592 to the requestednumber of significant figures.

a. 7 significant figures

b. 5 significant figures

c. 3 significant figures

16. Complete the following calculations. Round offthe answers to the correct number of significantfigures.

a. 2.30 m � 3.65 m � 0.55 m �

b. 103.8 m � 31 s �

c. 26.0 cm � 2.1 cm �

SUPPLEMENTAL PROBLEMSCHAPTER 2

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Supplemental Problems Chemistry: Matter and Change • Chapter 3 3

Matter—Properties and ChangesMatter—Properties and Changes1. An 18-g sample of element A combines com-

pletely with a 4-g sample of element B to formthe compound AB. What is the mass of thecompound formed?

2. A substance breaks down into three componentelements when it is heated. The mass of eachcomponent element is listed in the table below.What was the mass of the substance before itwas heated?

3. Silver iodide powder has been used as an anti-septic and as an agent to seed clouds for rain.Silver iodide is 45.9% silver by mass. If youseparate a 50-g sample of silver iodide into itselements, silver and iodine, how much silverwould you have?

4. If 5 g of element A combines with 16 g of ele-ment B to form compound AB, how manygrams of B are needed to form compound AB2?How many grams of B are needed to formAB3?

5. During a chemical reaction, 2.445 g of carbonreacts with 3.257 g of oxygen to form carbonmonoxide gas. How many grams of carbonmonoxide are formed in this reaction?

6. Ibuprofen has the chemical formula C13H18O2.It is 75.69% carbon, 8.80% hydrogen, and15.51% oxygen. How many mg of carbon doesa 200-mg tablet of ibuprofen contain?

7. During a chemical reaction, 4.032 g of hydro-gen combined with oxygen to form 36.032 g ofwater. How many grams of oxygen reacted?

8. Nitrogen and oxygen combine to form differentcompounds, as shown below.

What is the ratio of the masses of nitrogen ineach of the following?

NO2/NO4 �

NO/NO4 �

NO/NO2 �

9. Carbon and oxygen combine to form carbonmonoxide (CO) and carbon dioxide (CO2). Themasses of oxygen that combine with 12 g ofcarbon to form these two compounds are 16 gand 32 g, respectively. What is the ratio of themasses of oxygen in CO2/CO?

10. Phosphorus and chlorine combine to form twodifferent compounds. In one compound, 3.88 gof phosphorus combines with 13.28 g of chlo-rine. In the other compound, 1.32 g of phos-phorus combines with 7.56 g of chlorine. Dothese data support the law of multiple propor-tions? Show your work.

CompoundChemicalFormula Mass N/1 g O

Nitric oxide

Nitrogen dioxide

Nitrous oxide

NO

NO2

NO4

1.76 g

0.88 g

0.44 gComponent Mass (g)

A

B

C

39.10

54.94

64.00

SUPPLEMENTAL PROBLEMSCHAPTER 3

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4 Chemistry: Matter and Change • Chapter 3 Supplemental Problems

11. Fluorine and xenon combine to form two dif-ferent compounds. In one compound, 0.853 gof fluorine combines with 1.472 g of xenon. Inthe other compound, 0.624 g of fluorine com-bines with 2.16 g of xenon. Do these data sup-port the law of multiple proportions? Showyour work.

12. Ferric chloride is 34.4% iron and 65.6% chlo-rine by mass. A chemist analyzes three com-pounds that contain iron and chlorine. Herresults are summarized in the data table below.Which of these compounds is likely to be ferricchloride? Explain your answer.

13. The chemical formula for baking soda isNaHCO3. A 168.02-g sample of baking sodacontains 45.98 g of sodium, 2.02 g of hydro-gen, 24.02 g of carbon, and 96 g of oxygen.What is the mass percentage of each element inbaking soda?

14. The chemical formula for chalk is CaCO3.A100-g sample of chalk contains 40 g of cal-cium, 12 g of carbon, and 48 g of oxygen.What is the mass percentage of each element inchalk? What would be the mass of calcium in200 g of chalk?

15. A 17-g sample of ammonia, NH3, contains 3 gof hydrogen. What percentage of ammonia ishydrogen? How many grams of nitrogen doesthe sample contain?

CompoundMass of the Sample (g)

Mass ofFe (g)

Mass ofCl (g)

I

II

III

25

25

27

9.3

8.6

9.3

15.7

16.4

17.7

SUPPLEMENTAL PROBLEMSCHAPTER 3

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Supplemental Problems Chemistry: Matter and Change • Chapter 4 5

The Structure of the AtomThe Structure of the Atom1. Use the periodic table to complete the

following table.

2. Give the number of protons, electrons, and neutrons in each of the following atoms.

a. 10847Au

b. 4020Ca

c. 2311Na

3. Name each isotope, and write it in symbolicnotation.

a. atomic number 26; mass number 56

b. atomic number 29; mass number 64

c. atomic number 17; mass number 37

4. How many protons, electrons, and neutrons arein each of the following isotopes?

a. uranium-235

b. hydrogen-3

c. silicon-29

5. How many neutrons does europium-151 have?What is the isotope’s mass number?

6. How many more neutrons does thorium-230have than protons? How many electrons doesthorium-230 have?

7. Show that the mass number and the number ofprotons are conserved in the following nuclearequation: 234

92U 0 23090Th � 4

2He.

8. Give the mass number of each isotope.

a. Be with 5 neutrons

b. Ga with 39 neutrons

c. Si with 16 neutrons

d. Ti with 26 neutrons

9. Give the atomic number of each isotope.

a. magnesium-25

b. bromine-79

c. antimony-121

10. Neon has two isotopes: neon-10 and neon-12.

a. Which isotope has the greater mass?

b. Which has more neutrons?

c. Which has more protons?

d. Which has more electrons?

11. Use the table below to calculate the atomicmass of element X. Then use the periodic tableto identify the element. Show all your work.

Isotope Mass (amu) Percent Abundance

16X17X18X

15.995

16.999

17.999

99.762

0.038

0.20

ElementAtomicNumber Protons Electrons

a. Li

b.

c.

d. Hg

e.

f.

g. B

93

81

75

87

80

SUPPLEMENTAL PROBLEMSCHAPTER 4

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6 Chemistry: Matter and Change • Chapter 4 Supplemental Problems

12. Magnesium has three isotopes. Magnesium-24has a percent abundance of 78.99%.Magnesium-26 has a percent abundance of11.01%. What is the percent abundance ofmagnesium-25? Assume that there are no othermagnesium isotopes.

13. Calculate the atomic mass of iridium. Iridiumhas two isotopes. Iridium-191 has a mass of191.0 amu and a percent abundance of 37.58%.Iridium-191 has a mass of 193.0 amu and apercent abundance of 62.42%. Show all yourwork.

14. An element has three naturally occurring isotopes.

Isotope 1 has a mass of 19.992 amu.

Isotope 2 has a mass of 20.994 amu.

Isotope 3 has a mass of 21.991 amu.

The pie graph shows the relative abundance ofeach isotope.

a. Calculate the atomic mass of the element.

b. Identify the element, using the periodictable.

15. An element has three naturally occurring iso-topes. Information about each isotope is sum-marized below.

a. Find the atomic mass of this element. Showall your work.

b. Identify the element, using the periodictable.

c. Write each isotope in symbolic notation.

16. The isotope carbon-14 can be used to deter-mine the ages of objects that were once living,such as wood, bones, and fossils. While alive,living things take in all the isotopes of carbon,including carbon-14. Carbon-14 undergoesradioactive decay continuously. After an organ-ism dies, the carbon-14 in its body continues todecay. However, its body no longer takes innew carbon-14. Thus, by measuring how muchcarbon-14 a once-living object contains andcomparing it with the amount of carbon-14 in acurrently living thing, you can determine theage of the object.

a. In terms of subatomic structure, how doescarbon-14 differ from carbon-12 andcarbon-13?

b. How is carbon-14 like carbon-12 andcarbon-13?

c. Carbon-14 emits a beta particle as it decays.What atom does carbon-14 decay to?

d. Write an equation to represent the decay ofcarbon-14.

Isotope Mass (amu) Percent Abundance

Isotope 1

Isotope 2

Isotope 3

23.985

24.946

25.983

78.10

10.13

11.17

Isotope 190.51%

Isotope 39.22%

Isotope 20.27%

SUPPLEMENTAL PROBLEMSCHAPTER 4

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Supplemental Problems Chemistry: Matter and Change • Chapter 5 7

Electrons in AtomsElectrons in Atoms

SUPPLEMENTAL PROBLEMSCHAPTER 5

10. Complete the following table.

Element Symbol 1s

Orbitals ElectronConfiguration

a. Nitrogen

b.

c. Carbon

d.

F

1s22s22p3

1s22s1

2s 2px 2py 2pz

)( )( )( )( )

1. Orange light has a frequency of 4.8 � 1014 s�1.What is the energy of one quantum of orangelight?

2. Which is greater, the energy of one photon of orange light or the energy of one quantum of radiation having a wavelength of 3.36 � 10�9m?

3. Use the relationships E � h� and c � �v towrite E in terms of h, c, and �.

4. A radio station emits radiation at a wavelengthof 2.90 m. What is the station’s frequency inmegahertz?

5. Record the frequency of your favorite radiostation. What is the wavelength of the radiationemitted from the station?

6. List the sequence in which the followingorbitals fill up: 1s, 2s, 3s, 4s, 5s, 6s, 7s, 2p, 3p,4p, 5p, 6p, 7p, 3d, 4d, 5d, 6d, 4f, 5f.

7. Which element has the ground-state electronconfiguration [Kr]5s24d105p4?

8. Which element has the ground-state electronconfiguration [Ar]4s23d10?

9. Write electron-dot structures for the followingatoms.

a. [Ne]3s23p3

b. [Ar]4s23d3

c. potassium

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8 Chemistry: Matter and Change • Chapter 5 Supplemental Problems

12. Use the figure below to answer the followingquestions.

a. How many valence electrons does an atomof this element have?

b. What is the atom’s electron-dot structure?

c. If enough energy was added to remove anelectron, from which energy level would theelectron be removed? Explain your answer.

13. What is the ground-state electron configurationof each of the following atoms? Use noble-gasnotation.

a. selenium

b. krypton

c. chlorine

14. What is the highest energy level (n) that isoccupied in the following elements?

a. He

b. Ca

c. Sn

15. Write the electron configuration for each ele-ment described below and identify the element.

a. an element that contains 8 electrons

b. an element that contains 14 electrons

2e�

8e�8e�

2e�

SUPPLEMENTAL PROBLEMSCHAPTER 5

11. Complete the orbital diagram for arsenic.

2s2p

3s

3p

4s 3d

5p

4f

6p

5f

7p

5s4p

4d

6s5d

7s

6p

7p6d

5f

4f5d

4d

3d4p

3p

2p

6d

7s

5s

4s

3s

2s

1s

Incr

easi

ng

En

erg

y

6s5p

1s

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Supplemental Problems Chemistry: Matter and Change • Chapter 6 9

The Periodic Table and Periodic LawThe Periodic Table and Periodic LawFor questions 1–5, do not use the periodic table.

1. Write the electron configurations for the elements in periods 2–4 of group 2A.

2. Determine the group, period, and block of the elements with the following electron configurations.

a. [He]2s22p4

b. [Xe]6s1

c. [Ar]4s23d104p2

3. Categorize each of the elements in problem 2as a representative element or a transition element.

4. Write the electron configuration of the elementfitting each of the following descriptions. Usenoble-gas notations.

a. Group 8A element in the third period

b. Group 4A element in the fourth period

c. Halogen in the second period

d. Group 1A element in the fourth period

5. What are the noble-gas notations of all the ele-ments with the following valence electron con-figurations?

a. s2

b. s2p1

For questions 6–9, do not use Figure 6-12, 6-15,or 6-20.

6. Rank the following atoms in order of decreasing radii.

a. Al, Na, P, S

b. Al, Ga, In

c. As, Ge, Ga

d. Br, Ca, Cl, K

7. Rank the following ions in order of decreasingradii.

a. Br�, Cl�, F�

b. Be2�, Ca2�, Mg2�

c. Ca2�, Ga3�, K�

8. Rank the following particles in order ofdecreasing radii.

a. I, I�

b. K, K�

c. Al, Al3�

9. Rank the following atoms in order of decreas-ing electronegativity.

a. Na, Li, K

b. K, Sc, Ca

c. As, Sn, S

SUPPLEMENTAL PROBLEMSCHAPTER 6

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Supplemental Problems Chemistry: Matter and Change • Chapter 10 11

Chemical ReactionsChemical ReactionsBalance the following chemical equations.

1. SnS2(s) � O2(g) 0 SnO2(s) � SO2(g)

2. C2H6(g) � O2(g) 0 CO2(g) � H2O(g)

3. Al(s) � HCl(aq) 0 AlCl3(aq) � H2(g)

4. CoCO3(s) 0 CoO(s) � CO2(g)

Write a balanced equation for each of the follow-ing reactions, substituting symbols and formulasfor names. Include the state of each reactant andproduct. Then identify the reaction type for each.If more than one reaction type applies, list allthat apply.

5. When aluminum nitrate and sodium hydroxidesolutions are mixed, solid aluminum hydroxideforms. The other product is sodium nitrate.

6. When magnesium is heated in the presence ofnitrogen gas, solid magnesium nitride forms.

7. When solid copper(II) oxide and hydrogenreact, metallic copper and water form.

8. Most industrial production of metallic sodiumis accomplished by passing an electric currentthrough molten sodium chloride. Chlorine gasalso is produced.

9. Liquid pentane (C5H12) burns, producing watervapor and carbon dioxide.

10. When chlorine gas is passed through a potas-sium bromide solution, bromine forms in apotassium chloride solution.

11. Magnesium burns in air to form magnesiumoxide.

Predict the products in each of the followingreactions. If no reaction occurs, write NR. Youmay use Figure 10-10 for the relative activities ofcommon metals and halogens.

12. Rb(s) � CaCl2(aq)

13. Pt(s) � MnBr2(aq)

14. F2(g) � NaI(aq)

15. Zn(s) � AgNO3(aq)

Write a complete ionic equation and a net ionic equation for each of the following double-displacement reactions.

16. Ba(NO3)2(aq) � H2SO4(aq) 0BaSO4(s) � 2HNO3(aq)

17. FeCl3(aq) � (NH4)3PO4(aq) 0FePO4(s) � 3NH4Cl(aq)

18. KCl(aq) � AgC2H3O2(aq) 0AgCl(s) � KC2H3O2(aq)

SUPPLEMENTAL PROBLEMSCHAPTER 10

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Supplemental Problems Chemistry: Matter and Change • Chapter 11 13

The MoleThe Mole1. Identify and calculate the number of representa-

tive particles in each of the following quantities.

a. 2.15 moles of gold

b. 0.151 mole of nitrogen oxide

c. 11.5 moles of potassium bromide

2. Calculate the number of moles of the substancethat contains the following number of represen-tative particles.

a. 8.92 � 1023 atoms of barium

b. 5.50 � 1025 molecules of carbon monoxide

c. 2.66 � 1022 formula units of potassiumiodide

3. Determine the mass in grams of each of the following quantities.

a. 1.24 moles of beryllium

b. 3.35 moles of calcium

c. 0.155 mole of sulfur

4. Calculate the number of moles in each of thefollowing quantities.

a. 6.35 g lithium

b. 346 g zinc

c. 115 g nickel

5. How many atoms are in the following samples?

a. 1.24 g cobalt

b. 0.575 g cesium

c. 65.6 g silicon

6. Which quantity has the greatest mass?

a. 4.16 � 1023 atoms of radium

b. 1.50 � 1020 atoms of cadmium

c. 1.33 � 1024 atoms of argon

7. Calculate the number of moles in each of thefollowing quantities.

a. atoms of each element in 3.35 moles ofaspirin (C9H8O4)

b. positive and negative ions in 1.75 moles ofcalcium fluoride (CaF2)

8. Determine the molar mass of each of the following compounds.

a. formic acid (CH2O2)

b. ammonium dichromate ((NH4)2Cr2O7)

9. What is the mass in grams of each of the following quantities?

a. 2.53 moles of lead(II) nitrate (Pb(NO3)2)

b. 4.62 moles of magnesium bromide (MgBr2)

10. Calculate the number of moles in each of the following samples.

a. 3.75 g calcium carbide (CaC2)

b. 245 g aluminum nitrite (Al(NO2)3)

11. Determine the percent composition of each ofthe following compounds.

a. manganese oxide (MnO)

b. propanol (C3H8O)

c. calcium phosphate (Ca3(PO4)2)

SUPPLEMENTAL PROBLEMSCHAPTER 11

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14 Chemistry: Matter and Change • Chapter 11 Supplemental Problems

12. Determine the empirical formula for a 100.00-gsample of a compound having the followingpercent composition.

a. 94.07% sulfur and 5.93% hydrogen

b. 80.68% mercury, 12.87% oxygen, and6.45% sulfur

13. A 48.30-g sample of an aluminum-iodine com-pound contains 3.20 g of aluminum. What isthe empirical formula for the compound?

14. A 50.00-g sample of hydrated manganese(II)chloride yields 31.75 g of the anhydrous com-pound after heating. Determine the chemicalformula and name of the hydrate.

15. Caffeine is a compound found in some naturalcoffees and teas and in some colas.

a. Determine the empirical formula forcaffeine, using the following composition of a 100.00-g sample.

49.47 grams of carbon, 28.85 grams ofnitrogen, 16.48 grams of oxygen, and 5.20 grams of hydrogen

b. If the molar mass of caffeine is 194.19 g/mol, calculate its molecularformula.

SUPPLEMENTAL PROBLEMSCHAPTER 11

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Supplemental Problems Chemistry: Matter and Change • Chapter 12 15

StoichiometryStoichiometry1. Silicon nitride is used in the manufacturing of

high-temperature thermal insulation for heatengines and turbines. It is produced by the fol-lowing reaction.

3Si(s) � 2N2(g) 0 Si3N4(s)

a. Interpret the equation in terms of particles,moles, and masses.

b. Show that mass is conserved in the reaction.

2. The heat from a welder’s torch is produced bythe burning of acetylene gas. The reaction isrepresented by the following balanced chemicalequation.

2C2H2(g) � 5O2(g) 0 4CO2(g) � 2H2O(g)

Calculate the mole ratios from the balancedequation.

3. Limestone (CaCO3) is treated with hydrochlo-ric acid and water to manufacture calcium chlo-ride hexahydrate. This compound is used tomelt ice and snow on pavements and roads.The following balanced chemical equation rep-resents the reaction.

CaCO3(s) � 2HCl(aq) � 5H2O(l) 0CaCl26H2O(s) � CO2(g)

a. How many moles of calcium chloridehexahydrate will be produced from 4.00 mol calcium carbonate?

b. How many moles of hydrogen chloride willbe needed to produce 1.25 mol of thehydrate?

c. If 8.33 mol water is available for thereaction, how many moles of carbondioxide will be released?

4. To prevent corrosion and make paints adherebetter, some aluminum products are treatedwith chromium(III) phosphate before finishing.Chromium(III) phosphate (CrPO4) is commer-cially produced by treating chromium metalwith orthophosphoric acid (H3PO4).

a. Balance the following equation for thereaction.

Cr(s) � H3PO4(aq) 0

H2(g) � CrPO4(s)

b. How many moles of chromium metal areneeded to produce 855 g of chromium(III)phosphate?

c. The reaction of 206 g chromium willrelease how many moles of hydrogen gas?

5. Sand (silicon dioxide) and coke (carbon) arecombined to form silicon carbide (SiC), a com-pound used in high-strength ceramic materials.

a. Balance the following equation for thereaction.

SiO2(s) � C(s) 0

SiC(s) � CO(g)

b. What mass of silicon carbide will beproduced from the reaction of 352 g silicondioxide?

c. If 1.00 g of carbon is reacted, what mass ofcarbon monoxide is released?

SUPPLEMENTAL PROBLEMSCHAPTER 12

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16 Chemistry: Matter and Change • Chapter 12 Supplemental Problems

6. Two compounds of nitrogen, nitrogen tetroxide(N2O4) and hydrazine (N2H4), are used asrocket fuels. When the two compounds aremixed, they ignite spontaneously and producenitrogen gas and water.

a. Balance the following equation for thereaction.

N2O4(l) � N2H4(l) 0

N2(g) � H2O(g)

b. If 8.00 g nitrogen tetroxide and 4.00 ghydrazine are mixed, determine thefollowing quantities.

1. limiting reactant

2. mass of product (N2)

3. mass of excess reactant

7. One step in the industrial refining of nickel isthe decomposition of nickel carbonyl(Ni(CO)4) into nickel and carbon monoxide. Ina laboratory reaction, 25.0 g nickel carbonylyielded 5.34 g nickel.

a. Balance the following equation for thereaction.

Ni(CO)4(g) 0

Ni(s) � CO(g)

b. Determine the theoretical yield of nickel.

c. Determine the percent yield.

SUPPLEMENTAL PROBLEMSCHAPTER 12

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Supplemental Problems Chemistry: Matter and Change • Chapter 13 17

States of MatterStates of Matter1. Calculate the ratio of effusion rates of oxygen

(O2) to hydrogen (H2).

2. Methane (CH4) effuses at a rate of 2.45 mol/s.What will be the effusion rate of argon (Ar)under the same conditions?

3. The effusion rate of hydrogen sulfide (H2S) is 1.50 mol/s. Another gas under similar conditions effuses at a rate of 1.25 mol/s. What is the molar mass of the second gas?

4. The pressure of a gas in a manometer is 12.9 mm Hg. Express this value in each of the following units.

a. torr

b. atmosphere

c. kilopascal

5. The vapor pressure of water is 2.3 kPa at 23°C.What is the vapor pressure of water at this temperature expressed in atmospheres?

6. What is the pressure of a mixture of nitrogen(N2) and oxygen (O2) if the partial pressure ofN2 is 594 mm Hg and the partial pressure ofO2 is 165 mm Hg?

7. A sample of air is collected at 101.1 kPa. If thepartial pressure of water vapor in the sample is2.8 kPa, what is the partial pressure of the dryair?

8. Suppose that 5-mL containers of helium (He),neon (Ne), and argon (Ar) are at pressures of 1 atm, 2 atm, and 3 atm, respectively. The Heand Ne are then added to the container of Ar.

a. What is the partial pressure of He in thecontainer after the three gases are mixed?

b. What is the total pressure in the containerafter the three gases are mixed?

SUPPLEMENTAL PROBLEMSCHAPTER 13

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Supplemental Problems Chemistry: Matter and Change • Chapter 14 19

GasesGases1. In one city, a balloon with a volume of 6.0 L is

filled with air at 101 kPa pressure. The balloonin then taken to a second city at a much higheraltitude. At this second city, atmospheric pres-sure is only 91 kPa. If the temperature is thesame in both places, what will be the new volume of the balloon?

2. A certain mass of gas in a 2.25-L container has a pressure of 164 kPa. What will the newpressure be if the volume of the container isreduced to 1.50 L and the temperature staysconstant?

3. If 5.80 dm3 of gas is collected at a pressure of92.0 kPa, what volume will the same gasoccupy at 101.3 kPa if the temperature staysconstant?

4. If the volume of an air pump used to inflate a football decreases from 480 mL to 375 mL,and the original pressure was 93.5 kPa, what is the new air pressure in the pump if the temperature stays constant?

5. Maintaining constant pressure, the volume of agas is increased from 18.0 dm3 to 32.0 dm3 byheating it. If the original temperature was18.0°C, what is the new temperature in degreesCelsius?

6. A natural gas tank is constructed so that thepressure remains constant. On a hot day whenthe temperature was 33°C, the volume of gas inthe tank was determined to be 3000.0 L. Whatwould the volume be on a warm day when thetemperature is 11°C?

7. A 50.0-mL sample of gas is cooled from 119°Cto 80.0°C. If the pressure remains constant,what is the final volume of the gas?

8. A 10.0-L cylinder of gas is stored at room tem-perature (20.0°C) and a pressure of 1800 psi. Ifthe gas is transferred to a 6.0-L cylinder, atwhat Celsius temperature would it have to bestored in order for the pressure to remain at1800 psi?

9. If the gas pressure in an aerosol can is 148.5 kPa at 23°C, what is the pressure inside the can if it is heated to 298°C?

10. A tank for compressed gas has a maximum safepressure limit of 850 kPa. The pressure gaugereads 425 kPa when the temperature is 28°C.What is the highest temperature in degreesCelsius the tank can withstand safely?

11. In a steel container, it was found that the pres-sure of the gas inside was 160 kPa when thecontainer had been heated to 98°C. What hadbeen the pressure of the gas when the tempera-ture had been 50°C the previous day?

12. A steel cylinder is filled with a gas at a temper-ature of 25.0°C and a pressure of 225.0 kPa.What will the pressure be if the temperature israised to 47°C?

13. A balloon is filled with gas at a pressure of102.3 kPa and a temperature of 45.5°C. Its volume under these conditions is 12.5 L. Theballoon is then taken into a decompressionchamber where the volume is measured as 2.50 L. If the temperature is 36.0°C, what is the pressure in the chamber?

SUPPLEMENTAL PROBLEMSCHAPTER 14

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20 Chemistry: Matter and Change • Chapter 14 Supplemental Problems

14. A weather balloon contains 14.0 L of helium ata pressure of 95.5 kPa and a temperature of12.0°C. If this had been stored in a 1.50-Lcylinder at 21.0°C, what must the pressure inthe cylinder have been?

15. How many moles of a gas will occupy 2.50 Lat STP?

16. Calculate the volume that 3.60 g H2 gas willoccupy at STP.

17. What volume is occupied by 0.580 mol of gasat 98.4 kPa and 11°C?

18. When a sample of a gas was placed in a sealedcontainer with a volume of 3.35 L and heatedto 105°C, the gas vaporized and the resultingpressure inside the container was 170.0 kPa.How many moles of the gas was present?

19. An engineer wishes to design a container thatwill hold 14.0 mol of gas at a pressure nogreater than 550 kPa and a temperature of48°C. What is the minimum volume the container can have?

20. What is the molar mass of a sample of gas thathas a density of 2.85g/L at 101 kPa pressureand 29°C?

21. How many grams of gas are present in a sample that has a molar mass of 44 g/mol and occupies a 1.8-L container at 108 kPa and 26.7°C?

22. What is the molar mass of a gas if 142 g of thegas occupies a volume of 45.1 L at 28.4°C and94.6 kPa?

23. Determine the volume of hydrogen gas neededto make 8 L of water vapor.

24. Calculate the volume of chlorine gas at STPthat is required to completely react with 3.50 gof silver, using the following equation: 2Ag(s) + Cl2(g) 0 2AgCl(s).

25. Use the reaction shown to calculate the mass ofiron that must be used to obtain 0.500 L ofhydrogen at STP.

3Fe(s) � 4H2O(l) 0 Fe3O4(s) � 4H2(g)

SUPPLEMENTAL PROBLEMSCHAPTER 14

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Supplemental Problems Chemistry: Matter and Change • Chapter 15 21

SolutionsSolutions1. The solubility of a gas is 0.34 g/L at STP. What

is its solubility at a pressure of 0.80 atm andthe same temperature?

2. At 25°C and 1.0 atm, 0.25 g of a gas dissolvesin 1.00 L of water. What mass of the gas dis-solves in 1.00 L of water at 25°C and 3.0 atm?

3. 1.56 g of a gas dissolves in 2.00 L of water at apressure of 1.75 atm. At what pressure will2.00 g of the gas dissolve in 2.00 L of water ifthe temperature remains constant?

4. What is the percent by mass of 92.3 g of potassium fluoride (KF) dissolved in 1000.0 gof water?

5. A 500.0 g-sample of aqueous hydrogen perox-ide (H2O2) contains 31.50% H2O2 by mass.

a. Find the mass of hydrogen peroxide in thesolution.

b. Find the mass of water in the solution.

6. If 24.0 mL of methanol (CH3OH) is dissolvedin 48.0 mL of water, determine the percent byvolume of methanol in the solution.

7. An aqueous solution of methanol is 45.0%methanol by volume.

a. Find the volume of methanol in a 250.0-mLsample of the solution.

b. Find the volume of water in this sample ofthe solution.

8. What is the molarity of a solution that contains20.45 g of sodium chloride (NaCl) dissolved in700.0 mL of solution?

9. Calculate the molarity of 0.205 L of a solutionthat contains 156.5 g of sucrose (C12H22O11).

10. A 0.600-L sample of a 2.50M solution of potas-sium iodide (KI) contains what mass of KI?

11. What mass of ammonium chloride (NH4Cl)would you use to prepare 85.0 mL of a 1.20Msolution NH4Cl?

12. How would you correctly prepare 125 mL of a0.30M solution of copper(II) sulfate (CuSO4)from a 2.00M solution of CuSO4?

13. A 22.0-mL sample of 12M H2SO4 is diluted toa volume of 1200.0 mL. What is the molarityof the diluted solution?

14. A mass of 134 g of manganese dibromide(MnBr2) is dissolved in 225 g of water. What isthe molality of the solution?

15. Calculate the molality of a solution that con-tains 106 g naphthalene (C10H8) dissolved in3.15 mol carbon tetrachloride (CCl4).

16. A solution is made by dissolving 425 g of nitricacid (HNO3) in 535 g of water. Find the molefraction of nitric acid in the solution.

SUPPLEMENTAL PROBLEMSCHAPTER 15

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Supplemental Problems Chemistry: Matter and Change • Chapter 16 23

Energy and Chemical ChangeEnergy and Chemical Change1. Calculate the amount of heat released in the

complete combustion of 8.17 g of Al to formAl2O3(s) at 25°C and 1 atm. �Hf° for Al2O3(s)� �1680 kJ/mol.

4Al(s) � 3O2(g) 0 2Al2O3(s)

2. From the following data at 25°C,

H2(g) � Cl2(g) 0 2HCl(g) �H � �185 kJ

2H2(g) � O2(g) 0 2H2O(g) �H � �483.7 kJ

calculate �H at 25°C for the reaction below.

4HCl(g) � O2(g) 0 2Cl2(g) � 2H2O(g)

3. Determine �S for the reaction

SO3(g) � H2O(l) 0 H2SO4(l),

given the following entropies.

Compound Entropy (J/mol�K)

SO3(g) 256.8

H2O(l) 70.0

H2SO4(l) 156.9

4. Calculate the molar entropy of vaporization forliquid hydrogen iodide at its boiling point,�34.55°C.

HI(l) 7 HI(g) �Hvap � 19.76 kJ/mol

5. Ozone (O3) in the atmosphere may react withnitric oxide (NO).

O3(g) � NO(g) 0 NO2(g) � O2(g)

From the following data, calculate the �G° inkJ for the reaction at 25°C and determinewhether the reaction is spontaneous.

�H° � �199 kJ

�S° � �4.1 J/K

6. For the reaction H2(g) � S(s) 0 H2S(g), �H � �20.2 kJ and �S � 43.1 J/K. When willthe reaction be spontaneous?

7. The following reaction is nonspontaneous at25°C.

Cu2O(s) 0 2Cu(s) � �12� O2 (g)

�Hf° � 168.6 kJ

If �S � 75.8 J/K, what is the lowest tempera-ture at which the reaction will be spontaneous?

8. Calculate �H° at 25°C for the reaction below.

2ZnS(s) � 3O2(g) 0 2ZnO(s) � 2SO2(g)

�206.0 0 �350.5 �296.8�Hf°(kJ/mol)

9. How much heat is evolved in the formation of35.0 g of Fe2O3(s) at 25°C and 1.00 atm pres-sure by the following reaction?

4Fe(s) � 3O2(g) 0 2Fe2O3(s)

�Hf° (kJ/mol) 0 0 �824.2

10. Calculate the standard heat of vaporization,�Hvap, for tin(IV) chloride, SnCl4.

�Hf°� �511.3 kJ/mol for SnCl4(l) and �471.5 kJ/mol for SnCl4(g).

11. Given the following data at 298 K, calculate�S for the given reaction.

2Ag2O(s) 0 4Ag(s) � O2(g)

�S (J/mol�K) 121.3 42.6 205.2

SUPPLEMENTAL PROBLEMSCHAPTER 16

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24 Chemistry: Matter and Change • Chapter 16 Supplemental Problems

12. Calculate the �G° at 298 K for the followingreaction.

Fe2O3(s)�13CO(g) 0 2Fe(CO)5(g)�3CO2(g)

�824.2 �110.5 �733.8 �393.5�H° (kJ/mol)

87.4 197.6 445.2 213.6�S° (J/mol�K)

13. Estimate the temperature at which �G � 0 forthe following reaction.

NH3(g) � HCl(g) 0 NH4Cl(s)

�H � �176 kJ, �S � �284.5 J/K

14. Consider the reaction below at 25°C for which�S � 16.1 J/K.

CH4(g) � N2(g) � 163.8 kJ 0HCN(g) � NH3(g)

At what temperature will this reaction be spontaneous?

15. Estimate the temperature above which the following reaction is not spontaneous.

PbS(s) � 2HCl(g) 0 PbCl2(s) � H2S(g)

�100.4 �92.31 �359.4 �20.60�Hf° (kJ/mol)

�98.70 �95.30 �314.1 �33.60�G° (kJ/mol)

16. Copper metal has a specific heat of 0.385J/g�°C and a melting point of 1083°C.Calculate the amount of heat required to raisethe temperature of 22.8 g of copper from20.0°C to 875°C.

17. How many degrees of temperature rise willoccur when a 25.0-g block of aluminumabsorbs 10.0 kJ of heat? The specific heat ofaluminum is 0.897 J/g�°C.

18. Find the standard enthalpy of formation for eth-ylene, C2H4(g), given the following data.

C2H4(g) � 3O2(g) 0 2CO2(g) � 2H2O(l)

�H° � �1411 kJ

C(s) � O2(g) 0 CO2(g)

�H° � �393.5 kJ

H2(g) � �12� O2(g) 0 H2O(l)

�H° � �285.8 kJ

19. Glycine is important for biological energy. Thecombustion of glycine is given by the follow-ing equation.

4C2H5O2N(s) � 9O2(g) 08CO2(g) � 10H2O(l) � 2N2(g)

�H � �3857 kJ

Given that �Hf° CO2(g) � �393.5 kJ/mol and�Hf° H2O(l) � �285.8 kJ/mol, calculate theenthalpy of formation per mole of glycine.

20. At body temperature, 2404 J is required toevaporate 1 g of water. After vigorous exercise,a person feels chilly because the body is givingup heat to evaporate the perspiration. A typicalperson perspires 25 mL of water after 20 min-utes of exercise. How much body heat is usedto evaporate this water?

SUPPLEMENTAL PROBLEMSCHAPTER 16

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Supplemental Problems Chemistry: Matter and Change • Chapter 17 25

Reaction RatesReaction Rates

1. For the reaction BrO3� � 5Br� � 6H� 0

3Br2 � 3H2O, the value of �

1.5 � 10�2 mol/(L�s) at a particular time.

What is the value of at the same

instant?

2. The reaction, A � 2B 0 Products, was foundto have the rate law, Rate � k[A][B]2. Whileholding the concentration of A constant, theconcentration of B was increased from x to 3x.Predict by what factor the rate of the reactionwill increase.

3. For the hypothetical reaction A � B 0Products, the following initial rates of reactionhave been measured for the given reactant concentrations.

What is the rate law expression for this reaction?

4. For the chemical reaction H2O2 � 2H� �2I� 0 I2 � 2H2O, the rate law expression isRate � k[H2O2][I�]. The following mechanismhas been suggested.

H2O2 � I� 0 HOI � OH�

OH� � H� 0 H2O

HOI � H� � I� 0 I2 � H2O

Identify all intermediates included in this reaction.

5. Consider the following rate data for the reac-tion below at a particular temperature.

2A � 3B 0 Products

What is the rate equation for this reaction?

6. Consider a chemical reaction involving compounds A and B that is found to be firstorder in A and second order in B. What will the reaction rate be for experiment 2?

7. The data below were determined for the following reaction.

S2O82� � 3I� 0 2SO4

2� � I3

What is the rate equation for this reaction?

Experiment I� (M)Initial Rate (mol/(L�s))[S2O8

2�] (M)

1

2

3

0.10

0.20

0.20

0.40

0.40

0.20

1.4 � 10�5

2.8 � 10�5

1.4 � 10�5

ExperimentInitial [A] (M)

Initial[B] (M)

Rate (mol/(L�s))

1

2

0.10

?

1.0

2.0

0.2

0.6

ExperimentInitial[A] (M)

Initial[B] (M)

Initial Rate of Loss of A (mol/(L�s))

1

2

3

0.10

0.10

0.20

0.30

0.60

0.90

1.00 � 10�5

2.00 � 10�5

1.20 � 10�4

Test [A] (M) [B] (M) Rate (mol/(L�hr))

1

2

3

0.010

0.015

0.010

0.020

0.020

0.010

0.020

0.030

0.005

��[Br�]��

�t

��[BrO3�]

���t

SUPPLEMENTAL PROBLEMSCHAPTER 17

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26 Chemistry: Matter and Change • Chapter 17 Supplemental Problems

8. For the reaction A � B 0 C, the rate relation-ship is found to be Rate � k[A][B]2. What isthe overall reaction order for this reaction?

9. For the rate law expression Rate � k[A][B]2,what happens to the rate if the concentration ofB is increased by a factor of 2?

10. Calculate the specific rate constant for the reac-tion A � B 0 C, when the rate expression isRate � k[A]2[B].

11. The following figure shows the energy diagramof some reactants changing into products.Explain what the numbers in the diagram represent.

12. The following figure shows the potentialenergy diagram for a reaction. Explain whatthis diagram tells you about the reaction.

13. Explain how the following mechanism can beused to determine the rate expression for achemical reaction A � 2B 0 AB2.

Step 1 B � B 0 B2 slow

Step 2 B2 � A 0 AB � B fast

Step 3 B � AB 0 AB2 fast

14. What is the rate law expression for the following mechanism?

Step 1 AB � C2 0 AC2 � B slow

Step 2 B � AB 0 AB2 fast

Step 3 AC2 � AB2 0 A2C2 � B2 fast

Step 4 A2C2 � B2 0 A2C � B2C fast

Reaction progress

X � Y

Z � R

a

b

c

dPote

nti

al e

ner

gy

Reaction progress

40 kJ

100 kJ

Ener

gy

(kJ)

ExperimentInitial[A] (M)

Initial[B] (M)

Initial Rate of Formation of C

(mol/(L�s))

1

2

3

0.10

0.20

0.20

0.10

0.10

0.20

2.0 � 10�4

8.0 � 10�4

1.6 � 10�3

SUPPLEMENTAL PROBLEMSCHAPTER 17

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Supplemental Problems Chemistry: Matter and Change • Chapter 18 27

Chemical EquilibriumChemical Equilibrium1. Write equilibrium expressions for the following

reactions.

a. NH4HS(g) 3 NH3(g) � H2S(g)

b. 4HCl(g) � O2(g) 3 2Cl2(g) � 2H2O(g)

c. PCl5(g) 3 PCl3(g) � Cl2(g)

d. CuSO4�3H2O(s) � 2H2O(g) 3CuSO4�5H2O(s)

2. At 793 K, the equilibrium constant for the reac-tion NCl3(g) � Cl2(g) 3 NCl5(g) is 39.3.

a. Do products or reactants dominate in thisequilibrium?

b. If the equilibrium constant for this reactionwere less than 1, would the reactants orproducts be dominant?

3. At 773 K, the reaction 2NO(g) � O2(g) 32NO2(g) produces the following concentra-tions: [NO] � 3.49 � 10�4M; [O2] � 0.80M;[NO2] � 0.25M.

a. What is the equilibrium constant expressionfor the reaction?

b. What is the equilibrium constant for thereaction?

4. If you wished to maximize the products of thefollowing reactions, which concentrationswould you lower or raise?

a. H2(g) �Br2(g) 3 2HBr(g)

b. CO2(g) � H2(g) 3 CO(g) � H2O(g)

c. SO2(g) �NO2(g) 3 SO3(g) � NO(g)

d. C(s) � CO2(g) 3 2CO(g)

5. For each reaction, state whether increasing ordecreasing the volume of the reaction vesselwould yield more product at equilibrium. Givethe reason for your choice.

a. N2O4(g) 3 2NO2(g)

b. 2SO3(g) 3 2SO2(g) � O2(g)

c. CH4(g) � 2O2(g) 3 CO2(g) �2H2O(g)

d. 2CO(g) � O2(g) 3 2CO2(g)

6. What effect would an increase in temperaturehave on these reactions at equilibrium? Why?

a. Heat � H2(g) � I2(g) 3 2HI(g)

b. CH4(g) � 2O2(g) 3 CO(g) � 2H2O � heat

c. N2(g) � 3H2(g) 3 2NH3(g) � heat

d. Heat � CH4(g) 3 C(s) � 2H2(g)

7. Phosphorous pentachloride decomposes tophosphorous trichloride according to this equation: PCl5(g) 3 PCl3(g) � Cl2(g).At equilibrium, [PCl5] � 1.00M and [Cl2] �3.16 � 10�2M.

a. Write the expression for determining theconcentration of PCl3.

b. What is the equilibrium concentration ofPCl3? Use: Keq � 1.00 � 10�3.

8. The solubility product constant (Ksp) ofAg2SO4 is 1.2 � 10�5.

a. How would you estimate the molarsolubility of SO4

2� without actuallycalculating it?

b. What is the calculated molar solubility of SO4

2�?

SUPPLEMENTAL PROBLEMSCHAPTER 18

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Supplemental Problems Chemistry: Matter and Change • Chapter 19 29

Acids and BasesAcids and BasesWrite balanced chemical equations for each ofthe following reactions that involve acids andbases.

1. aluminum and hydrochloric acid

2. nitric acid and sodium carbonate

3. potassium hydroxide and sulfuric acid

Write the steps in the complete ionization of thefollowing polyprotic acids.

4. H2CO3

5. H3BO3

A solution has a [H�] of 1.0 � 10�5M.

6. What is its [OH�]?

7. What is its pH?

8. What is its pOH?

A solution has a [OH�] of 3.6 � 10�7M.

9. What is its [H�]?

10. What is its pH?

11. What is its pOH?

A solution has a [H�] of 5.6 � 10�6M.

12. What is its [OH�]?

13. What is its pH?

14. What is its pOH?

A solution has a pH of 5.79.

15. What is its pOH?

16. What is its [H�]?

17. What is its [OH�]?

18. What is the pH of a 0.50M solution of HCl, astrong acid?

19. What is the pH of a 1.5 � 10�3M solution ofNaOH, a strong base?

20. What is the molarity of a KOH solution if 25.0 mL of it is neutralized by 31.7 mL of a0.100M nitric acid solution?

21. During a titration, 0.200M HCl is added to aNaOH solution of unknown concentration.What is the concentration of the NaOH solutionif 20.0 mL of it is neutralized by 30.7 mL ofthe standard solution?

22. A 25.0-mL sample of H2SO4 is neutralized by27.4 mL of 1.00M KOH. What is the concen-tration of the acid?

23. A 50.0-mL sample of 0.0100M Ca(OH)2 is neu-tralized by 45.6 mL of HBr. What is the molar-ity of the acid?

SUPPLEMENTAL PROBLEMSCHAPTER 19

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Supplemental Problems Chemistry: Matter and Change • Chapter 20 31

Redox ReactionsRedox ReactionsDetermine the oxidation number of the boldfaceelement in these ions.

1. HgCl4�

2. NO2

3. MnO2

4. metallic Au

5. Na2SiF6

6. Zn(NO3)2

7. Mg3P2

8. Na3PO4

9. H2O2

10. ClO3�

Balance the following equations, using the oxida-tion number method for the redox part of theequation. Show your work.

11. Cu2O(s) � H2(g) 0 Cu(s) � H2O(l)

12. Cl2(g) � KBr(aq) 0 Br2(l) � KCl(aq)

13. CaSi2(s) � SbCl3(s) 0Sb(s) � Si(s) � CaCl2(s)

14. KI(aq) � HNO3(aq) 0I2(s) � KNO3(aq) � NO(g) � H2O(l)

15. Cr2O72�(aq) � SO3

2�(aq) 0Cr3�(aq) � SO4

2�(aq) in an acidic solution

Write half-reactions for each of the followingredox reactions. Identify each half-reaction asbeing either oxidation or reduction.

16. SnS2(s) � O2(g) 0 SnO2(s) � SO2(g)

17. Mg(s) � N2(g) 0 Mg3N2(s)

18. Al(s) � Cl2(g) 0 AlCl3(s)

19. NH3(aq) � PbO(s) 0N2(g) � Pb(s) � H2O(l)

20. Cu2S(s) � O2(g) 0 Cu2�(aq) � SO42�(aq)

(Hint: Two different elements are oxidized.)

Use your answers for questions 16–20 to help you balance the following equations, using half-reactions for the redox part of the equation.Show your work.

21. SnS2(s) � O2(g) 0 SnO2(s) � SO2(g)

22. Mg(s) � N2(g) 0 Mg3N2(s)

23. Al(s) � Cl2(g) 0 AlCl3(s)

24. NH3(aq) � PbO(s) 0 N2(g) � Pb(s) � H2O(l)

25. Cu2S(s) � O2(g) 0 Cu2�(aq) � SO42�(aq) in

an acidic solution (Hint: Look at the ratio ofthe two oxidized elements in the equation.)

SUPPLEMENTAL PROBLEMSCHAPTER 20

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Supplemental Problems Chemistry: Matter and Change • Chapter 21 33

ElectrochemistryElectrochemistryUse data from Table 21-1 as needed in the following problems. Assume that all half-cells are under standard conditions.

1. For each of these pairs of half-reactions, writea balanced equation for the overall cell reactionand calculate the standard cell potential, E0

cell.

a. Cs�(aq) � e� 0 Cs(s)

Cu�(aq) � e� 0 Cu(s)

Cell reaction:

E0cell �

b. Hg2�(aq) � 2e� 0 Hg(l)

Mn2�(aq) � 2e� 0 Mn(s)

Cell reaction:

E0cell �

c. Fe3�(aq) � 3e� 0 Fe(s)

Cr3�(aq) � 3e� 0 Cr(s)

Cell reaction:

E0cell �

d. Br2(g) � 2e� 0 2Br�(aq)

Au�(aq) � e� 0 Au(s)

Cell reaction:

E0cell �

e. Be2�(aq) � 2e� 0 Be(s)

Tl3�(aq) � 3e� 0 Tl(s)

Cell reaction:

E0cell �

f. NO3�(aq) � 4H�(aq) � 3e� 0

NO(g) � 2H2O(l)

In3�(aq) � 3e� 0 In(s)

Cell reaction:

E0cell �

g. H3PO4(aq) � 2H�(aq) � 2e� 0H3PO3(aq) � H2O(l)

SeO42�(aq) � 4H�(aq) � 2e� 0

H2SeO3(aq) � H2O(l)

Cell reaction:

E0cell �

h. MnO4�(aq) � 8H�(aq) � 5e� 0

Mn2�(aq) � 4H2O(l)

2CO2(g) � 2H�(aq) � 2e� 0 H2C2O4(aq)

Cell reaction:

E0cell �

2. Calculate the standard cell potential, E0cell, for a

cell composed of a Sn�Sn2� half-cell and eachof these half-cells.

a. Pd�Pd2�

E0cell �

b. Hf �Hf 4�

E0cell �

c. Cl2�Cl�

E0cell �

d. Pb�Pb2�

E0cell �

3. Which of the following cells will produce thehighest voltage?

Mn �Mn2��Zn2��Zn

Zn �Zn2��Ni2��Ni

Ni � Ni2��Cu2�� Cu

SUPPLEMENTAL PROBLEMSCHAPTER 21

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34 Chemistry: Matter and Change • Chapter 21 Supplemental Problems

4. For each of these overall cell reactions, writethe oxidation and reduction half-reactions, cal-culate the standard cell potential, E0

cell, anddetermine if the reaction is spontaneous or not.

a. Fe3�(aq) � Co2�(aq) 0Fe2�(aq) � Co3�(aq)

Oxidation half-reaction:

Reduction half-reaction:

E0cell �

Spontaneous?

b. Fe3�(aq) � Cu�(aq) 0Fe2�(aq) � Cu2�(aq)

Oxidation half-reaction:

Reduction half-reaction:

E0cell �

Spontaneous?

c. 3Ni2�(aq) � 2Rh(s) 03Ni(s) � 2Rh3�(aq)

Oxidation half-reaction:

Reduction half-reaction:

E0cell �

Spontaneous?

d. 2Na�(aq) � 2Hg(l) � 2I�(aq) 0 2Na(s) � Hg2I2(s)

Oxidation half-reaction:

Reduction half-reaction:

E0cell �

Spontaneous?

e. O2(g) � 2H2SO3(aq) 02SO4

2�(aq) � 4H�(aq)

Oxidation half-reaction:

Reduction half-reaction:

E0cell �

Spontaneous?

5. Suppose a battery-powered device requires aminimum voltage of 9.0 V to run. How manylead–acid cells would be needed to run thedevice? (Remember that a standard automobilebattery contains six lead–acid cells connectedin one package.) The overall reaction of alead–acid cell is

Pb(s) � PbO2(s) � 4H�(aq) � 2SO42�(aq)

0 2PbSO4(s) � 2H2O(l)

6. What is the minimum voltage that must beapplied to a Down’s cell to cause the electroly-sis of molten sodium chloride? The net cellreaction is

2Na�(l) � 2Cl�(l) 0 2Na(l) � Cl2(g)

7. One way to determine the metallic compositionof an alloy is to use electroplating. Suppose anelectrolytic cell is set up with solution of nickelions obtained from a 6.753-g sample of anickel alloy. The cell also contains a platinumelectrode that has a mass of 10.533 g. Electriccurrent is used to reduce the nickel ions tonickel metal, which is deposited on the plat-inum electrode. After being plated with nickel,the platinum electrode has a mass of 15.042 g.What is the percentage of nickel in the alloy?

SUPPLEMENTAL PROBLEMSCHAPTER 21

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Supplemental Problems Chemistry: Matter and Change • Chapter 22 35

HydrocarbonsHydrocarbons1. Use the IUPAC rules to name the following

alkanes.

a. CH3CH2CH2CH2CH3

b.

c.

d.

2. Draw the structure of each of the followingalkanes.

a. 4-propyloctane

b. 3,4-diethylhexane

c. 2,2,4,4-tetramethylhexane

d. 1-ethyl-3-methyl-2-propylcyclopentane

3. Calculate the number of hydrogen atoms ineach of the following alkanes.

a. heptane

b. cyclooctane

4. Calculate the molecular mass of a 22-carbonbranched-chain alkane.

5. Chemists can analyze the composition ofhydrocarbons by reacting them with copperoxide. The reaction converts carbon into carbondioxide and hydrogen into water. Suppose 29 gof a hydrocarbon reacts to produce 88 g of CO2and 45 g of H2O.

a. What are the masses of carbon andhydrogen in the hydrocarbon?

b. What is the empirical formula of thehydrocarbon?

c. If the hydrocarbon’s molecular mass is 58 amu, what is its molecular formula?

6. Carbon has an electronegativity of 2.5.Hydrogen has an electronegativity of 2.2. Usethese values to decide whether each of the following bonds is polar or nonpolar.

a. C-C

b. C-H

c. H-H

7. The combustion of a saturated hydrocarbonreleases 657 kJ per mole of –CH2– groups and779 kJ per mole of –CH3 groups in the hydro-carbon. How much energy is released by thecombustion of 1.00 L of liquid tetradecane(molecular formula C14H30), a major compo-nent of kerosene? The density of tetradecane is0.764 g/mL.

CH3CH3

CH2CH3

CH2CH3

CH3CH2

CH3

CH2CH3

CH2CH3

CH3CH2CHCHCHCH2CH3

CH3

CH3

CH3CHCHCH3

CH3

SUPPLEMENTAL PROBLEMSCHAPTER 22

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36 Chemistry: Matter and Change • Chapter 22 Supplemental Problems

8. Use the IUPAC rules to name the followinghydrocarbons.

a. CH3CH2CH�CHCH3

b.

c.

d.

9. Draw the structure of each of the followinghydrocarbons.

a. 7-methyl-2,5-nonadiene

b. 4-ethyl-2-heptyne

c. 1,2-diethylcyclohexene

d. 1-ethyl-2-methyl-5-propylbenzene

10. Calculate the number of hydrogen atoms ineach of the following unsaturated hydrocarbons.

a. 2-pentene

b. 1-hexyne

11. Write a balanced equation for the reaction inwhich calcium carbide, CaC2, reacts with waterto form ethyne and calcium hydroxide.

CH2CH3

CH3

CH3CHCH2CH2C�CH

CH3

CH3CH2CH2CHCH2CH2CH2CH3

CH�CH2

SUPPLEMENTAL PROBLEMSCHAPTER 22

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Supplemental Problems Chemistry: Matter and Change • Chapter 24 37

The Chemistry of LifeThe Chemistry of Life1. Calculate the molecular masses of the follow-

ing biological molecules.

a. Lysine, NH2(CH2)4CHNH2COOH

b. Fructose, CH2OHCO(CHOH)3CH2OH

c. Oleic acid,CH3(CH2)7CH�CH(CH2)7COOH

2. Write a balanced equation for the condensationreaction in which cysteine and glycine combineto form a dipeptide. Assume the carboxyl groupof cysteine reacts.

3. In a peptide or protein that contains n aminoacids, the number of possible amino acidsequences is An, where A is the number of dif-ferent amino acids.

a. How many amino acid sequences arepossible for a polypeptide that contains 10 amino acids?

b. How many different dipeptides can be madefrom the amino acids leucine (Leu) andvaline (Val)? What are those dipeptides?

4. Write a balanced equation for the condensationreaction in which lauric acid, palmitic acid, andstearic acid combine with glycerol to form atriglyceride.

CH3(CH2)10COOH CH3(CH2)14COOHlauric acid palmitic acid

CH3(CH2)16COOHstearic acid

5. In saponification, the ester bonds of a triglyc-eride are hydrolyzed by a strong base, such asNaOH. It takes 3 moles of NaOH to saponifyeach mole of triglyceride. How many moles oftriglyceride can be saponified by 120 g ofNaOH?

6. A young adult male produces about 2.4 � 10�5

mol per day of the steroid sex hormone testos-terone. The molecular mass of testosterone is288. How many grams of testosterone per daydoes a young adult male produce?

7. Synthesizing fats is an efficient way for organ-isms to store energy. The catabolism of 1 g offat yields about 38 kJ of energy, whereas thecatabolism of 1 g of protein or carbohydrateyields about 17 kJ of energy.

a. How much carbohydrate would be neededto store the same amount of energy as 10 gof fat?

b. A cup (133 g) of ice cream contains about32 g of carbohydrate, 4.8 g of protein, and14 g of fat. How much energy is releasedwhen a cup of ice cream is fullycatabolized?

c. A person expends about 840 kJ per hourwhile walking at a moderate pace. Howlong would a person have to walk to expendall of the energy contained in a cup of icecream?

8. A scientist analyzes a sample of DNA and findsthat 21% of the nucleotide bases are A and 29%of the bases are C. What percentage of thebases are T and what percentage are G in thesample?

SH

CH2

H2N C C

O

OH

H

cysteine

H

H2N C C

O

OH

H

glycine

SUPPLEMENTAL PROBLEMSCHAPTER 24

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38 Chemistry: Matter and Change • Chapter 24 Supplemental Problems

9. It takes three consecutive nucleotides in a DNAmolecule to code for one amino acid in a pro-tein. If a single strand of DNA contains 747nucleotides, how many amino acids would bein the protein that it codes for?

10. The DNA in a bacterial cell contains about 4.2 � 106 complementary base pairs. Each basepair has an average length of 3.4 � 10�10 m.How long is the DNA in a bacterial cell?Assume that the DNA is stretched out straightrather than coiled.

11. One mole of ATP stores approximately 30.5 kJof energy. This energy is released when ATP ishydrolyzed.

a. Approximately 38 moles of ATP isproduced for each mole of glucose that iscatabolized in cellular respiration. Howmuch energy is stored in ATP when 5.0 moles of glucose is catabolized incellular respiration?

b. Assume that 40% of this energy can be usedto drive anabolic reactions when ATP ishydrolyzed. The rest will be lost as heat.How much energy will be lost as heat if allof the ATP produced in part a is hydrolyzed?

12. A scientist performed an experiment to monitorphotosynthesis by a plant. In the experiment,the plant produced 61 g of glucose.

a. How many moles of glucose did the plantproduce?

b. How many moles of O2 did the plantproduce?

c. How many moles of CO2 were needed toproduce that much glucose?

d. What mass of water was needed to producethat much glucose?

13. An average-sized woman produces about 1900 g of carbon dioxide per day.

a. How many moles of glucose must beoxidized during cellular respiration toproduce that much carbon dioxide?

b. How much energy would be stored in ATPwhen that much glucose is oxidized?

14. Suppose the catabolism of a given amount ofglucose produces 95 moles of ATP during cel-lular respiration. How many moles of ATPcould be produced by the same amount of glu-cose during fermentation?

15. How many grams of glucose are needed to produce 102 g of ethanol during alcoholic fermentation?

16. Write a balanced equation for lactic acid fer-mentation. The formula for lactic acid isCH3CH(OH)COOH.

SUPPLEMENTAL PROBLEMSCHAPTER 24

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Supplemental Problems Chemistry: Matter and Change • Chapter 25 39

Nuclear ChemistryNuclear ChemistryWrite a complete nuclear equation for each ofthe following.

1. The decay of 5326Fe by beta emission.

2. The decay of 23090Th by alpha emission.

3. The decay of 3718Ar by electron capture.

4. The decay of 3819K by positron emission.

5. The decay of 9343Tc by gamma emission.

Provide the missing term in each of the followingequations.

6. 115B � 4

2He 0 147N �

7. 4520Ca � 1

1p 0 4521Sc �

8. 157N � 0 18

8O � 11p

9. 23392U � 1

0n 0 9942Mo � 31

0n �

10. 0 20682Pb � 4

2He

11. 14258Ce � 0 142

59Pr � 10n

12. 10244Ru � 4

2He 0 10n �

Answer the following questions about half-life.

13. The half-life of 11551Sb is 32 minutes. How much

of a 16.0-g sample of this isotope will remainat the end of 3.0 hours?

14. The half-life of 18272Hf is 9.0 � 106 years. How

much of a 1.0-g sample of this isotope willremain at the end of 40.0 million years?

15. The isotope strontium-90 is produced duringthe testing of nuclear weapons. If 100.0 mg of strontium-90 was released in the atmosphere in 1960, how much of the radioisotope remains 85 years later? The half life of strontium-90 is29 years.

16. The radioisotope technetium-99 is often used asa radiotracer to detect disorders of the body. Ithas a half-life of 6.01 hours. If a patientreceived a 25.0-mg dose of this isotope duringa medical procedure, how much would remain48.0 hours after the dose was given?

SUPPLEMENTAL PROBLEMSCHAPTER 25


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